Process for purifying hydrogen and preparing carbonyl sulfide



United States Patent l 3,382,043 PROCESS FOR PURHFYING HYDROGEN AND PREPARING CARBONYL SULFIDE Edward A. Swakon, Hammond, Ind., assignor to Standard Oil Company, Chicago, Ill., a corporation of Indiana No Drawing. Filed June 12, 1963, Ser. No. 287,182 5 Claims. (Cl. 23-210) ABSTRACT OF THE DISCLOSURE Carbon monoxide is separated from mixtures of hydrogen and carbon monoxide gases and hydrogen gas of at least 90% purity can be recovered. The separation is accomplished by reacting the gas mixture with sulfur and a secondary amine or a mixture of secondary and tertiary amines in a reaction zone under conditions generating carbonyl sulfide in situ and retaining all the carbonyl sulfide in a secondary amine or tertiary amine salt of the monothiolcarbamic acid of the secondary amine by maintaining the salt under pressure and withdrawing from the reaction zone a gas of at least 90? hydrogen content.

This invention relates to the recovery of hydrogen and more particularly pertains to a method for the recovery of hydrogen from gaseous mixtures of hydrogen and carbon monoxide.

Many processes have been proposed for the production of hydrogen. Some commercial processes for the production of hydrogen are the steam-hydrocarbon process, water gas process, producer gas process and other similar processes, which produce a mixture containing hydrogen and carbon monoxide. Such mixtures of hydrogen and carbon monoxide, after removal of sulfur compoundsrare'usefti for example in the 0x0- process for converting olefins td aldliydes and"mixturesof aldehydes and alcohols. However, these mixtures of hydrogen and carbon monoxide are also useful as sources of hydrogen after removal of carbon monoxide. Commercially, the carbon monoxide is generally removed by converting it to carbon dioxide as, for example, through the reaction of carbon monoxide with water at about 700 F. This reaction:

does produce additional hydrogen but also produces carbon dioxide which must be removed from the various admixtureswith hydrogen.

-l mhods of converting carbon monoxide to carbonyl sulfide by reaction with sulfur followed by reaction of CO5 with primary amines and ammonia either as a separate step or at the same time as reacting CO and S to produce urens, have been devised. There are other reactions of carbonyl sulfide which would make this compound a valuable starting material if available in commercial quantities. In our research laboratories, it has been found that secondary amines or mixtures of secondary amines and tertiary amines will react with carbonyl sulfide to form secondary or tertiary amine salts of monothiol carbamic acid derivatives of the secondary amine. It has also been discovered in our laboratories that the reaction of carbon monoxide, sulfur and secondary amine or a mixture of secondary amine and tertiary amine will also form the secondary or tertiary amine salt of the monothiol carbamic acid derivative of the secondary amine. In either case, the amine salt of the monothiol carbamic acid is stable at temperatures not exceeding about 120 to 130 C when maintained under pressure.

It has also been found that carbonyl sulfide can be 3,382,043 Ice Patented May 7, 19

reacted at 0 to 100 C. with two moles primary amine to form the primary amine salt of the monothiolcarbamic acid of the primary amine or with one mole of primary amine and one mole of secondary or tertiary amine in which case a secondary amine salt or tertiary amine salt of the monothiolcarbamic acid of the primary amine forms. Also, carbonyl sulfide reacts with one mole of primary or one mole of secondary amine in the presence of a b asictorm of sodium, potassium, calcium, barium, magnesium, zinc, lead and mercury in which case the sodium, potassium, barium, magnesium, zinc, lead or mercury salt of the monothiolcarbamic acid corresponding to the primary or secondary amine forms.

Carbonyl sulfide can react with ammonia to form ammonium monothiolcarbamate in an alcohol, e.g., methanol or ethanol. However, at temperatures above 40 C. ammonium monothiolcarbamate decomposes to a mixture of urea, H 8, COS and ammonia which mixture in and of itself is not very useful.

In any of the foregoing processes of forming thiolcarbamates there is great flexibility in the choice of amine reactants to form the monothiolcarbamic acid and L e-just as great a flexibility in the choice of the amine or metal to form the salt. The amine salts of the mono-W thiolcarbamic acids from especially secondary amines will rapidly decompose at to C. and atmospheriu-g-f'fj pressure to carbonyl sulfide and secondary amine. The metal salts of the monothiolcarbamic acids are useful gw as intermediates, or as vulcanization accelerators, the

water soluble salts can be used to form vulcanizable rub her latices and the water insoluble salts, e.g. calcium, magnesium, zinc, lead and mercury salts can be used in solid vulcaniza'ble compositions.

For the formation of the salt of the monothiolcarbamic acid and substantially complete utilization of COS or CO, there is employed at least two moles of' i the same amine or at least one mole of primary orflg sgnfli secondary amine and one mole of tertiary amine or said basic form of metal for each mole of COS or CO. When x 7- the amine monothiolcarbamate formation and dccomposition are to be used toaasorb' and regenerate COS, it is desirable to use the secondary amine or mixtures of secondary and tertiary amines and to use these amines in excess of the aforementioned proportions. For the purpose of absorbing and regenerating COS, the presence of excess amines is of no consequence since the amines are recovered and recycled.

In the formation of monothiolcarbamates, it has further been observed in our laboratories that the absorption of COS or consumption of CO is substantially complete and quite rapid under conditions which are readily adaptable to commercial operation. Also the regeneration or liberation of COS from the amine monothiolcarbamate is substantially complete and rapid under conditions which are readily adaptable to commercial operations. For example, when the amine monothiolcarbamate is formed by reacting CO, S and a secondary amine or mixture of secondary amine and tertiary amine at temperatures of from 50 to C. and under pressure, COS is liberated rapidly and substantially quantitatively at 90 to 120 C. So if this reaction is carried out at 90 to 150 C. in the presence of sulfur and at a suitable pressure above atmospheric pressure in a closed system until the stoichiometric amount of CO is absorbed and the resulting mixture is depressurized while maintaining the mixture at 90 to 120 C., the amine monothiolcnrbamate decomposes to a mixture of CO8 and amine or mixture of amines. This COS-amine mixture can be passed through a partial condenser to recover the amine or mixture of amines and then the,

3 COS can be .separately condensed. If more than a stoichiomctric proportion of CO is charged, the CO-COS mixture remaining after condensing the amine or amines, is separated by condensing COS and recycling the CO.

Utilizing the rapid reaction of CO, S and a secondary 5 amine or a mixture of a secondary amine and tertiary amine and the rapid liberation of COS from the resulting amine monothiolcarbamate, we have devised a process for recovering hydrogen from mixtures containing hydro gen and carbon monoxide. By this process, the mixture In of hydrogen and carbon monoxide is reactec l \yi t l;i s t 1Eur; and said amines, mixtures of amines and mixtures of basic forms of metals and amines each in the proportions to carbon monoxide hereinbefore set forth. Suitably the reaction is carried out at an elevatedtenmggiupgab qye 50 C., desirablWC. so that carbonyl sulfide can be ge.. ed as a valEible by-product, and at an elevated pressure above atmospheric pressure, suitably at the autogcnetic pressure sum of the partial pressures of the amine, hydrogen and CO at reaction temperatures and desirably at a pressure of from 90 to 4500 p.s.i.g. It will be appreciated that at the end of a batch reaction the pressure will be much lower than at the beginning. However, even in a batch reaction with the gas containing both hydrogen and carbon monoxide being fed continuously until the stoichiometric proportion of CO is consumed, the reaction pressure can be maintained at no greater than the sum of the partial pressures of hydrogen and other gases associated therewith and the amine.

In a continuous process, the gas containing the H CO mixture is passed, in countercurrent relationship under pressure to a mixture of sulfur and secondary amine or sulfur with secondary amine and tertiary amine. This is conveniently accomplished by pumping the amine-sulfur mixture into the top of a reaction vessel such as a tubular reactor, packed tower such as scrubbing tower, or an extraction tower or similar to a tray or packed distillation tower or some other means for contacting a liquid and a gas, charging the gas containing H and CO at the bottom under pressure withdrawing at the bottom under pressure a liquid etliuent containing the amine-monothiolcarbamate, withdrawing at the top enriched hydrogen gases of reduced CO content and recycling these gases to remove all the CO or charging these withdrawn gases to a second reaction vessel to be contacted with an amine-sulfur mix- 4; ture or an amine-basic metalsulfur mixture. Or if economics are against such recycling or second reaction of the withdrawn hydrogen enriched gaseous mixture with these amounts of CO even up to 5 to 10 mole percent CO, this gaseous mixture can be contacted with ammonical cuprous salt solution or contacted with steam at 700 F. to convert the CO to CO and the CO scrubbed out with amine. However, a second reaction of the enriched hydrogen gas with additional amine-sulfur or amine-sulfur-basic form of metal will remove substantially all of the carbon monoxide.

The hydrogen-carbon monoxide gas mixture used in the process of this invention need not be pretreated to remove hydrogen sulfide or water. Hydrogen sulfide can be removed by conventional means from the hydrogen stream produced. The hydrogen produced by the process of this invention can be dried by conventional methods as, for example, by compressing and cooling, by treatment with liquid desiccants such as dicthylene glycol in admixture vith trimethylatniue, triethylamine, tripropylamine, etc fl idvantageously, when a mixture of secondary and tertiary amine is employed their boiling points should be closely related such as diisopropylamine and triethylamine, di-n-butylamine and tri-n-propylamine, diisoamylamine and triisobutylamine, etc. But since COS boils (and, hence, condenses) at much lower temperatures than the secondary amines or tertiary amines, the closeness of boiling points of secondary and tertiary amines is not critical. Secondary amines such as methylcyclohexyl amine, dicyclohexylamine, ethylphenylamine, dibenzyl- 7 amine, diphenylamine, among other secondary amines not strictly di alkyl amines can be used but to no particular advantage. In fact, for this hydrogen recovery process, the use of such secondary amines as dialkylamines containing 1 to 20 carbon atoms in each of their alltyl hydrocarbon groups do provide definite advantages, for their corresponding amine monothiolcarbamates are liquid products. Of these secondary amines, di-n-btuylamine is preferred, for its liquid amine monothiolcarbamate product. As will be hereinafter demonstrated, COS can be readily recovered from the liquid amine monothiolcarbamate product.

For a clearer understanding of the process of this invention, the following illustrative examples are given.

Example 1 A 300 ml. stainless steel reactor is charged with 100 g. (0.75 mole) di-n-butylaminc, 10.7 g. (0.33 mole) sulfur and 2000 p.s.i.g. CO/H (SS/42%) and heated to 200 F. After two hours, the temperature is maintained at 200 F. and gas samples taken at various pressures and analyzed. The amount of COS in vent gas is measured by an Orsat apparatus. It is assumed that the absorption of gas in di-n-butylamine is due to COS, however, the amine also would pick up H S and CO Cut Pressure, p.s.i.g. COS

The gas removed by depressurizing to 1700 p.s.i g. is substantially only hydrogen.

The reactor is next connected to a Dry Ice-acetone trap and heated to 240 F. and 16 g. of theory) of COS is recovered. This COS plus that in the gas vented from below 1700 to 180 p.s.i.g. accounts for substantially all of the COS produced.

Example 2 Another process is .carriedput similar to Example 1 except reaction tcmperafinc is 140 F. After one hour at reaction temperature (final pressure was 1500 p.s.i.), gas samples are taken at various pressures and analyzed by Orsat method using di-n-butylamine and by mass spectroscopy from which the following analyses were obtained:

' Pressure, Percent Percent Cut p.s.i.g. COS Orsat COS mass spectroscopy These analyses show good agreement hetlgeen Orsat and mass spectroscopic analytical methods and demonstrate that nearly all of COS is retained in the amine solvent at this temperature (l tz of liquid condensed from vent gases in Dry lce acetone trap). The gas vented from 1500 to 250 p.s.i.g. at 140 F. is substantially all hydrogen. The reaction solution is transferred at atmospheric pressure to a round-bottom flask connected to reflux condenser fitted with outlet to Dry ice-acetone trap. The flask is heated and at about C. gas evolution is noted. Upon further heating to 120 C., about of COS comes over at -110 C. with 15.8 g. of COS collected at 100-120" C. Substantially all of the COS produced from carbon monoxide is recovered.

Example 3 In this example the reaction is conducted with excess sulfur to see how completely CO can be removed from a mixture containing 58% CO and 42% H A 300 ml. stainless steel reactor is charged with 20.8 g. sulfur, 100

- 5 g. di-n-butylamine and 1500 p.s.i. CO/H (SS/42%) mixture. Reaction is maintained at 138-150 F. for 1% hours. Final pressure at 138 F. is 825 p.s.i. (room temperature, 625 p.s.i.g.). Mass spectroscopic analysis of vent gas shows:

Gas: Percent About 91% of CO is consumed when operating at 1500 p.s.i. CO/H and 140 F. There is still considerable amount of sulfur left.

Example 4 The rate of uptake of CO from CO/H mixture is determined. A 300 ml. stainless steel reactor is charged with 100 g. di-n-butylamine and 16 g. sulfur, heated to 150 F. and then charged with 200 p.s.i.g. CO/Hg (H 42.0%; C0, 57.7%; CO 0.3%). A final pressure of 90 p.s.i.g. is reached in about 60 minutes in substantially a straight line relationship of pressure v. time. Mass spectroscopic analysis of the vent gas shows:

6 Percent H 93.6 C 6.2 CO 0 1 COS O 1 This demonstrates that about 95% of the CO is con- 0 sumed producing hydrogen of 93.6% purity.

Example 5 The process of Example 4 is repeated with 200 psi. of the same CO/H mixture but at 160 F. and rate of CO uptake is again followed. The pressure dropped to about 95 p.s.i.g. in minutes. The following vent gas analysis by mass spectroscopy is obtained:

Gas:

Again, high purity hydrogen is produced.

Example 6 Rate of CO uptake is again followed by repeating Example 4, charging the reactor with 500 psi. CO/Hg and heating to 150 F. From a plot of pressure versus reaction time it is found that the reaction rate is much faster at higher pressures. Even after the partial pressure of CO reaches the level of Examples 4 and 5, the rate o reaction is faster. This suggests that the monothiolcarbamate has a positive effect on the rate. Analysis of the vent gases at the end of the run shows:

Gas: Percent This demonstrates that of CO is consumed and hydrogen of 93% purity is produced.

Example 7 carbamate and then levels off in this case at about 0 pfs.i. g.,;the final pressure in all six reactions. Because all the reaction goes to 0 p.s.i.g., the amine must be holding all the formed COS as the di-n-butylamine salt of N-dibutylmonothiolcarbamic acid.

The process of this invention illustrated in Examples 1 through 7 has the following advantages. The secondary amine is an excellent solvent for sulfur, particularly under the reaction temperature conditions. When the secondary amine is employed as a solvent alone or together with a tertiary amine, reaction temperatures below those employed when other solvents such as methanol are cm ployed. Also, the eoh'W'fsion of carbon monoxide and sulfur to carbonyl suliide is substantially quantitative. In addition, carbonyl sulfide is absorbed substantially as rapidly as it is produced. This is a great advantage over previously used solvents where carbonyl sulfide is pro- .uced and vented from the reaction site with other gaseous materials. It will be appreciated that because carbonyl sulfide is absorbed substantially as rapidly as it is produced, overall reaction pressure is lower, but even more important, it is possible to operate at lower pressures than heretofore possible with other solvents. For example, when solvents other than secondary amines or mixtures of secondary and tertiary amines are employed, the reaction pressures at reaction temperatures of from 50l50 C. are in the range of 200- 1x1400 p.s.i.g. due to the high vapor pressure of carbonyl sulfide. When the amine solvents are employed, reaction 0 pressures as low as 0 p.s.i.g. and no higher than about p.s.i.g. (as is indicated by the final pressure in the illustrative batch processes) under the preferred conditions are obtained because there is substantially no carbonyl sulfide present to add its vapor pressure to the carbon monoxide and/or hydrogen. Furthermore, the process of this invention as hereinbcfore illustrated eliminates the requirement for recovering carbonyl sulfide from vent gases in admixture with hydrogen, carbon monoxide, and the like as by scrubbing or condensing carbonyl sulfide with liquid air, nitrogen or some other extremely low-temperature refrigerant to fractionally condense carbonyl sulfide from the vent gases.

For a continuous process a mixture of carbon monoxide and hydrogen and an amount of secondary amine such as di'outyl, diamyl, di'aexyl, dioctyl amine or of a mixture of secondary and-imiiary amine are charged to a reaction zone containing sulfur at 50 to 150 C. The mole ratio of total amine to Hg/CO gas is in the range of 2.0 to 2.2 moles amine per mole of CO. Sulfur is added to the reaction zone to maintain an excess over the amount of CO charged. Sulfur addition can be conveniently made by adding sulfur to the amine and preheating the amine to reaction temperature and pressure. A pressure in the range of 0 to 150 p.s.i.g. is maintained in the reaction zone by venting unrcacted gas through a pressure reducer when pressures above atmospheric are employed. The liquid reaction mixture amine monothiolcarbamate is withdrawn and maintained at at least its thermal decomposition temperature up to 250 F. In any case it is preferred to thermally decompose the amine rnonothiolcarbamate in the liquid phase, i.e. maintain the amine product of decomposition as a liquid. The carbonyl sulfide liberated is collected as a liquid either by cooling or by compressing and cooling.

The unreacted gas if the carbon monoxide content is higher than desired, is charged to a second reaction zone with sulfur and secondary amine or a mixture of secondary and tertiary amine under the same reaction conditions as hereinbefore set forth to remove substantially all of the carbon monoxide.

Two reaction zones in series with each zone having its own feed of amine and sulfur and with the source of carbon monoxide and hydrogen being fed to the first zone and gases vented from the first zone charged as gas feed to the second reaction zone should provide an unreacted To illustrate the utilization of other amines the follow- 7 ing examples are given.

Example 8 A mixture of hydrogen and when monoxide CO) is charged into the bottom of a tower into tlte top of which is charged a solution of sulfur in dihexylamine at 50 C. The mole ratio of di-nexylamine to carbon monoxide is 2 to 1 and the mole ratio of sulfur to carbon monoxide is 1.05 to l. The tower pressure is maintained at about 45 p.s.i.g. The gas retention time is up to about 30 minutes. The gases leaving the packed tower pass through a liquid separator. The liquid is returned to the tower and the gas is vented through a pressure reducer. Liquid is withdrawn from the bottom of tower through pressure reducer heated to 100 C. at atmospheric pressure in a vessel fitted with a condenser to recover COS as a liquid condensate. Liquid amine is pumped from the monothiolcarbamate decomposition vessel to sulfur dissolving tank from which it is charged with cooling to 50 C. to the top of the packed tower. By this process 95% and above of the carbon monoxide may be converted to carbonyl sulfide and high purity hydrogen gas, 93-95% or higher hydrogen, may be recovered from the top of the gas-liquid disengaging zone.

Example 9 The process of Example 8 is repeated except that dihcxylamine is eplace-ti tr an equimolecalar mixture of di-n-butylamine and tri-n-butylamine. By this process 95% and above of the CO may o converted to COS and high purity hydrogen, 93 to 95% and above may be obta ned.

The use of methylaniline in the process of this invention for most cfiicicnt operation requires that the process be carried out at pressures above atmospheric, e.g. 20 to 300 p.s.i.g., at temperatures in the range of 50 to 150 C. for the mention of the COS formed as the methylaniline salt of the corresponding N-mcthyl-N-phcnyl monothiolcar' amic acid is too low at atmospheric pressure. The use of diethanolamine at 30 C. and atmospheric pressure in the process of this invention also results in the contamination of the hydrogen stream withdrawn with COS. The retention of CO3 as the diethanolamine salt of N-bis(beta-hydroxyethyl) monotbiolcarbamic acid improves somewhat at 50 C. and atmospheric pressure and at pressures of 20 to 100 psi. and temperatures of 50 to 100 C. the retention of COS in the reaction mixture is suitable. Dicyclohexylamine absorbs the COS formed in situ at atmospheric pressure and to C. as do piperidine and morpholine, however, at these temperatures the corresponding amine monothiolearbamates are solids and their successful use in the process of this invention requires the use of either a solvent such as an alcohol. ketonc, water. liquid hydrocarbon. dibutylcther, dimethylformatc, tetrahydroitu'aa. dimethyl sulfoxide and chlorobenzene, among others or the use of equimolar portions of a tertiary amine of another secondary amine which will maintain the amine monothiolearbanute as a liquid.

Suitable mixtures of secondary and tertiary amines include. am ng others, mixtures of diand tributylaminc: diandfiamylamincs; diand trihcxylamines; diand trioctylamincs: dibutylamine and triethylaminc: dipropylamine and pyridine: dibutylaminc and dimcthylanilinc'. diethylamirze and pyridine; morpholine and tributylamine, tricthylamine. tripropylamine or trimetirylantinc; methylaniline and dimethylaniline; mcthylaniline and trimethylamine, triethyiamine. tripropylamincs or tributylarnines; dihexylamines r. d tributylamines: and dicyclohexylamine and trimethylamrnc, trietlaylamine. tripropylamines and tributylamines. Such mixtures may be suitably employed i atmospheric pressure at commercially feasible rates.

The following example will sullice for the illustration of the use of mixtures of secondary and tertiary amines.

Example 10 A 150 milliliter gas absorption vessel is charged with 0.3 mole grams) of tributylamine and 0.284 mole (36.7 grams) of di-n-butylamine containing 0.5 mole (16 grams) sulfur at 50 C. The pressure reducing valve for the venting gases is set at 30 p.s.i.g. A mixture of carbon monoxide and 40% hydrogen is introduced into the amine-sulfur reaction mixture until about 0.26 mole of carbon monoxide is introduced. The liquid reaction mixture whica forms liberates quantitatively the COS formed in situ and retained as the tributylamine salt of N-(di-n-butyl) moriothiolcarbarnic acid at to 125 C. and atmospheric pressure. By this process there may be obtained at the vent gas during reaction a hydrogen stream of to and above purity.

Th plocess of this invention is suitable for removal of carbon monoxide as low as 1% from a hydrogenconta ining. gas or as much as 99% CG and 1.0% H The process of this invention can be employed to remove carbon monoxide from gases vented from an axe process to provide hydrogen of sul'hcient purity for the reduction of the oxogenation aldehyde product. Also, the process of this invention is useful for carbon monoxide removal from mixtures of carbon monoxide and hydrogen available from steel mills and petroleum refineries in addition to carbon monoxide from the oxidation of hyd ocarbons with oxygen or water and from Water gas reactions.

What is claimed is:

1. A method of recovery of hydrogen from mixtures of hydrogen and carbon monoxide which comprises reacting at a temperature in the range of 5 to C., and at a 7 pressure in the range of Lfltoiltlfi ptmospher es,said mix ture containing hyt ogetiiliid earbo ri nionoxidein a reaction zone with sufilraii'difliqufi phase of an initial seconda'r'yhminrin"tiff amount to provide at least one mole of the sccontary amine per mole of carbon monoxide to thereby form the monothiolcarbamie acid of said secondary amine, said reaction being also in the additional presence of at least one mole of secondary amine, tertiary amine, or 'a mixture of secondary and tertiary amines, to thereby form the amine salt, corresponding with said additional amine or amines, of said monothiolcarbamic acid of the initial secondary amine, maintaining a pressure to retaiujn that salt all of the carbonylsulfide formed l im. and .vit hdraujngwthcaunreactgd.gas.fromsaid i ction zone whereby hydrogen of at least 90 mole percent purity is obtained.

2. A method of reco cry of hydrogen from mixtures of hydrogen and carbon monoxide which comprises reacting, at a temperature in the range of 50 to 150 C. and under pressure in the range of 1.0 to 300 atmospheres. said m xture of hydrogen and carbon monoxide with sulfur dissolved in a liquid phase of a dialkylamine whose alltyl groups contain 1 to 20 carbon atoms and in an amount of sulfur and the dialkylamine to provide one mole sulfur and two moles of that secondary amine per mole of carbon monoxide thereby forming a liquid phase of the dialkylamine salt of the Ndialkyl monothiolcarbamic acid of the dialkylarninc reactant, maintaining a pressure to retain in the liquid phase of the salt all the carbonyl sulfide formed in situ. withdrawing the unreacted gas mixture from said reaction Zone and recycling it to said reaction zone until the CO is consumed, and

9 thereafter withdrawing substantially carbon monoxide free hydrogen.

3. A method of recovery of hydrogen from mixtures of hydrogen and carbon monoxide which comprises reacting said mixture containing hydrogen and carbon monoxide in a reaction zone with sulfur dissolved in dibutylamine wherein the solution contains for each mole of carbon monoxide at least one mole of sulfur and two moles of dibutylamine per mole of carbon monoxide to form a liquid phase of dibutylamine salt of N-dibutylmonothiolcarbamic acid at a temperature in the range of from 50 to 120 C. and at a pressure to maintain a liquid phase of said salt and retain all carbonyl sulfide formed in situ in said salt, withdrawing the unreacted gas mixture from said reaction zone as hydrogen of about 90% purity, withdrawing said liquid phase of the amine monothiolcarbamate from the reaction zone, heating the withdrawn amine monothiolcarbamate to a temperature in the range of 90 to 120 C., collecting carbonyl sulfide liberated at 90 to 120 C., and recycling to the reaction zone the amine mixture residue remaining after carbonyl sulfide liberation.

4. The process of claim 3 wherein the hydrogen gas removed from the reaction zone is charged to a second reaction zone containing dibutylamine solution of sulfur UNITED STATES PATENTS 1,685,733 9/1928 Uhde 23-2 2,311,342 2/1943 Kerns et a1 232 X 2,486,778 11/1949 Doumani 232 2,524,088 10/1950 Shaw 232 2,758,005 8/1956 Oakley 23203 2,992,896 7/1961 Applegath et a1. 23203 3,125,417 3/1964 Franz et al. 23203 FOREIGN PATENTS 341,584 1/1931 Great Britain.

OSCAR R. VERTIZ, Primary Examiner.

B. H. LEVENSON, Assistant Examiner. 

